The Microwave Spectrum and Structure of Chlorofluoromethane

The Microwave Spectrum and Structure of Chlorofluoromethane...
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VOl. 75


The Microwave Spectrum and Structure of Chlorofluoromethane1 BY NORBERT MULLER~ RECEIVED OCTOBER 8, 1952 The microwave spectra of CH2C13jF and CHzC13'F between 16,100 and 39,000 Mc. have been measured and analyzed. The rotational parameters are a = 41,810.1 Mc., b = 5,715.7 Mc., G = 5,194.6 Mc., and a = 41,738.2 Mc., b = 5,580.5 Mc., c = 5,081.6 Mc., respectively. The structural parameters, calculated with an assumed value of 111'56' for the H-C-H angle, are = 1.078 =t 0.005 A., rcci = 1.759 f 0.003 A., I C F = 1.378 f 0.006 A. C1-C-F = 110'1' f 2', 0 = 125'41' f 5', where 0 is the angle between the C-Cl bond and the projection of the C-H bonds on the symmetry plane. From the hyperfine structure of the 10,1-11,0transition, the quadrupole coupling constants were evaluated as x s = -52.18 f 1 Mc., T h = 38.83 5 1 Mc. With certain assumDtions. this leads to a value of 6.6% for the per cent. double-bond character of the ,_C-CI bond. ~

The structures of the various chlorine- and fluorine-substituted methanes. were investigated by Brockway3 using electron diffraction. Recently, more precise structures of many of these derivatives have been obtained from their microwave spectral4providing a better basis for discussion of the bonding involved. The present study adds CHzClF to this list; in addition to the structure, the spectrum yields information about the distribution of charge in the molecule, through the quadrupole hyperfine structure, and a limited amount of information concerning the direction of the dipole moment. The sample of CHzClF studied was the gift of Dr. D. E. Kvalnes of the Jackson Laboratory of E. I. du Pont de Nemours and Company, and is gratefully acknowledged. An infrared spectrum was obtained with the Baird recording spectrometer; comparison with the spectrum published by Plyler and Lamb5 indicated that no further purification was necessary. The microwave spectrum was observed with a Stark modulation spectrograph6using 100 kilocycle square wave modulation. Frequencies were measured by means of harmonics of a 5 Mc. standard frequency monitored by beating with station WWV; they should be accurate to 0.1 Mc. except where otherwise stated. Analysis of the Spectrum.-Calculations based on approximate structural parameters showed that the molecule is a nearly prolate-symmetric top (K -0.97). with the dipole largely along the axis of the intermediate moment of inertia, or b-axis, although the possibility of an appreciable component along the axis of the least moment (a-axis) could not be excluded. Using the methods of King, Hainer and Cross,' whose notation is also adopted, it was possible to predict that the only strong lines between 16,000 and 30,000 Mc. would form transitions with A J = rt 1 and AK = 7 1(K = K-1) and J = 4 or greater. In addition there should be a series of lines with A J = 0 and AK = 1, extending upwards in frequency from about 35,000 Mc.


(1) The research reported in this paper was made possible by support extended Harvard University by the Office of Naval Research under O.N.R. Contract N5ori-76, Task Order V. (2) Shell Oil Company Predoctoral Fellow. (3) L. 0. Brockway, J . P h y s . Chem., 41, 186 (1937). (4) D. R. Lide, Jr., TIIIS JOURNAL, 74, 3548 (19521, and references given there. (5) E . K. Plgler and M. A. Lamb, J. Research N a f l . Bur. Standards, 45, 204 (1950). (6) K. B. McAfee, Jr.. R.H. Hughes and E. B. Wilson, Jr., Res. Sci. Instvumenls, 20, 821 (1949). (7) G. W. King, R. ? V I . Hainer and P. C. Cross, J . Chem. P k y s . , 11, 27 (1948).

As a result of the interaction of the chlorine nuclear quadrupole moment with the molecular rotation, all lines involving J's less than about twenty should resolve into hyperfine components. This hyperfme structure proved to be the means of identifying the observed transitions, a task which would otherwise have been nearly impossible in view of the great density of lines in the spectrum. A convenient starting point for the calculation of the hyperfine structure is the formula for the firstorder interaction energy8

+ + +



Here p = {"/4 C(C 1) - I ( I l)J(J l)]/ Z ( 2 1 - 1) ( 2 1 - 1) ( 2 1 3), with C = F ( F 1) - 1(1 1) - J ( J 1))where F is the quantum




number of the resultant of J and I . xs = eQPV/ W ,where s is, in turn, each of the three principal axes of inertia. The x's are experimentally determined, with the restriction that their sum be zero. The A's are the line strengths of the Q-branch transitions J , T ++ J , T' allowed when the dipole moment is along the axis designated by the superscript. Ordinarily, in applying this formula to an asymmetric top, the A's must be found by interpolating in the table^.^ However, Lidelo has recently derived expressions for the line strengths of slightly asymmetric rotors, which may be substituted in this formula and which readily give explicit equations for the quadrupole energy with corrections in the first order for the asymmetry; second-order asymmetry corrections could also be obtained at the expense of a great deal more effort. This method was used to check the equations derived previously, to the second order, by Knight and Feld'l; they are repeated here to the first order because the original equations contain a misprint involving the sign of the first-order term. Knight and Feld's work was used to estimate the magnitudes of the second-order asymmetry corrections, which are found to be less than 4% for J ' s up to twenty; since no second-order quadrupole theory is available, it is hardly justified to include these. The equations for the various cases and near prolate symmetry are (8) See J. K. Bragg, Phys. Re%, 74, 533 (1948). (9) P. C. Cross, R. hl. Hainer and G. W. King, J. Chem. P h y s . , 12, 210 (1944). (10) D. R. Lide, Jr., ibid., 20, 1761 (1952). (11) G. Knight, Jr., and B. T. Feld, Technical Report 8123, Research Laboratory of Electronics, Massachusetts Institute of Technology, 1949.


Feb. 20, 1953


f ( J , n ) = $JZ

- n21(J + 1)2 - n2

and the asymmetry parameter b =


+ 1 ) / ( ~- 3) = (c - b)/[2a - ( b + c)]

With a single quadrupolar nucleus of spin I = 3/2, the general multiplet obtained whenever J is a t least two for both levels of the transition consists of nine components if AJ = 1, or ten if AJ = 0. However, the intensities of the four components with AF = AJ are far greater than those of the remaining ones if J is four or higher. Further, numerical calculations show that in the present instance, the four strong componepts will usually coincide in pairs, giving those lines which resolve a t all the appearance of doublets. The main exception to this is the case of the very low J Q-branch lines, where the h y p e r h e multiplets will be quite complex. These expectations are confirmed by the observed spectrum, which contains a large number of doublets in addition to a number of more complicated patterns a t high frequencies. Particularly helpful in identifying the spectrum was the presence of about a dozen doublets with spacings on the order of 6 Mc., since it could be deduced from the equations using estimated x’s that such wide splittings could occur only for transitions with K = 1 c--) K = 2. The appearance of so many of these transitions in the K-band results from the rather unusual circumstance that, because of the asymmetry, a curve of these frequencies plotted as a function of J passes through a maximum in the middle of the band. Only one of the widely split doublets resolved further, into a quadruplet, as would be expected for the lowest J’s of the series; it could therefore be assigned with some confidence to the transition 82,~91,9 of CH2ClS6F. The Q-branch lines could


also be fairly readily identified from the predicted fine structure, furnishing parameters that led to the identification of the remaining lines with J’s up to twenty. The importance of the quadrupole effects in arriving a t and confirming assignments cannot be overrated, since the spectrum is heavily populated and there are few lines with low enough J’s to make the centrifugal distortion so small that unambiguous assignments could be made on the basis of frequency alone. The presence of the hyperfine structure on all the low J lines had the drawback, however, of making it impracticable to observe any resolved Stark effects, and so obtain quantitative data on the dipole moment. A careful search for lines resulting from the selection rules active if there is a dipole component along the a-axis had completely negative results, so i t may be concluded that the dipole moment is within a few degrees of the b-axis. (The b-axis lies within one degree of the bisector of the C-F-Cl angle; the a-axis also lies in the symmetry plane, while the c-axis is perpendicular to it.) The rotational parameters of the two isotopic species are given in Table I. Table I1 gives the observed frequencies and the frequencies calculated from these parameters; the latter calculations are made to the nearest megacycle, after which the quadrupole structure, computed to the nearest 0.01 Mc. is superimposed, so that the predicted and observed h e structure may also be compared. The quadrupole calculations are based on parameters evaluated from the l0,~-11,0 transition; these are Xa = -52.18 Me., Xb = 38.83 Me. each *1 Mc. The limits of error express the fact that the observed frequencies lead to more than enough equations to determine the parameters, and the results of using various groups of equations differ by about a megacycle. TABLE I ROTATIONAL PARAMETERS OF CHLOROFLUOROMETHANE a

b c

CHzCla’F, Mc.

CHzC13’F, Mc.

41,810.1 5,715.7 5,194.6

41 ,738.2 5,580.6 5,081.6

Structural Parameters.-The moments of inertia derived from the relations I , = 505,446.5/a1 etc., are displayed in Table 111. The six moments do not suffice to fix the structure of the molecule beIb cause of the equality of the combination I a ICfor the two isotopic species, which makes it possible to find only five of the six necessary independent parameters. The H-C-H angle immediately suggests itself as the one to be assumed a priori, first because the lightness of the hydrogen atoms makes the moments relatively insensitive to their exact location, and secondly because the measured H-C-H angle varies very little between CH2C12 and CH2F2 (see ref. 4) and would be expected to have an intermediate value here. It must be borne in mind, however, that the limits of error for the CH2Fz value are given as f25’, so that the assumed value of 111’56’ for the present compound cannot be supposed subject to a much smaller uncertainty. The distance between the hydrogen atoms is given by the explicit equation m H d 2 H H = I, I b - I,. The



Vol. 75


862 TABLE I1

MICROWAVE LINES OF CH2C1F A. Assigned transitions The frequencies marked with a's were measured under conditions which make them subject to errors up to 1 Mc. Observed frequency


Calculated frequency

16,487.12 16,492.71 17,648.07 17,652.92 18,916.70 18,961.29 18,967.52 19,232.16 19,917.48 19,919.07 20,011.22 20,016.47 20,619.17 20,620.26 20,621.30 21 ,084.05 21,090.31 21,429.80 21,437.05 21,596.35 21,600.0" 21,603.23 21,608.5 36,616.50 w 36,621.13 36,620.92 36,624.40 w 36,624.27 36,651.41 W 36,652.7T w 36,657.07 36,657.47" 1 0 , l - l 1.u 37 W 36,660.75" 36,660.56 36,663.42" W 36,663.19 37,129.14" 37,129.70' W w 37,133.04 37,132.67" 37,136.67 W 37,136.25" M 20.2-21.1 35 37,140.00 ) 37,140.00" W 37,146.66" 37,146.13 M 37,149.76 37,149.50 37,153.09 W 37,153.50" 37,158.82" 37,158.30' 20.2-21,1 37 W 37,166.20" W 3o.a-31.2 37 37,924.77" W 37,930.0" ........ 37,938" 3o.a-31.2 35 37,940.52' W \v ........ 37,950" ........ 37,952' W * These frequencies do not include quadrupole structures; overlapping of the isotopic multiplets and experimental difficulties in measuring the frequencies made it impossible to assign individual hyperfine components.



37 37 3.5 33

35 35 37

1 1


35 37 35 37 37 37

35 37 37




InIn-. IntenstenstensFrequency ity Frequency ity Frequency ity 21,966.23 M 25,708.51 M 16,117.91 Mc S 22,234.17 M 26,257.63 W 16,166.58 W 22,251.93 W 26,368.30 W 16,296.9" W 22,253.07 W 26,429.08 M

16.419.80 W 17,228.62 M 17,331.76 W 17,416.50 W 17.782.62 S 17.783.68 S 17.978.22 S 18.229.29 S 18.381.82 S 18,382.50 S 18,584.59 W 19.076.34 M 19,273.78 W 19,316.96 M 19,400.74 S 19.447.26 S 19,624.74 M 19.640.67 S 19.687.12 W 19,868.76 S 20,042.38 s 20.143.55" W 20,285.534W 20.469.5" W 21,053.4" M 21.298.60 S 21.626.6" w 21,915.40 M 21.965.24 M

22.443.0' W 22.446.6" W 22,564.64 M 22,892.11 W 22,919.28 hf 23.088.58 M 23,154.47 S 23.158.02 M 23,408.54 M 23,+50.31 W 23,452.00 W 23,602.58 S 23,703" W 23,711.04 S 23,727.50' W 23,883.90 M 24,105.38 M 24,250" W 24,345.15 S 24,349.08 S 24,349.84 s 24.Y28.22 W 25.082.26 W 25,088.20 W 25,197.90 W 25,214.92 W 25,819.82 if 25,628.67 W 25,707 52 11

26,551.16 26,616.38 26,617.97 26,920.64 27,138.5' 27.781.00 27,869.96 28,008.22 28.007.90 28,462.5" 28,526.33 28,746.70 28.887.99 29,252.29 29.358.15 29,463.66 29,658.40 29,925.4" 29,926= 29,997.2" 30,iooD 30.219.4" 30.220.7n 30,290.67 30,292' 30,580.73 30,645' 30,659.9' 30,837.8'




w M M hf



w W hf

IntensFrequency ity

30,843.59 S 30,992.18 M 31,023.24 M 31,509.67 S 31,535.33 M 31,887.8' W 31,822.92 M 31,924.32 M 32,479.50 S 33,051.68 M 33,057.8" W 33,162.40 M 33,224.05 M 33,404.40 M 33,406.00 M 33,633.04 M 33,677.98 M 33,733.21 S 33,769.71 S 33.787.00 S 36.583.05" W 36,585.2" W 36,587 57' W 36,631" W 37,914 ni 37,957a W 37.962.7fY M 38,198' M 38,199.27' h1 38,423.18"M 38.928.22n nr 39.021.44"M 39,028.46' h.I


remaining parameters were obtained by a technique


of successive approximations; the limits of error are those resulting from the uncertainty of about half a


f c n = 1.078 f 0.005 A.

degree in the H-C-H angle. The best values are


0.003 A.


= 1.759


= 1.378 f. 0.006 A.


= 111"56' f 30' by assumption LCl-C-F = 110'1' xk 2' e = 125041' i Y

Feb. 20. 1953


where B is the angle between the C-Cl bond and the projection of the C-H bonds on the symmetry plane. For comparison, the parameters derived f;om electron diffraction3 are ~ C C I= 1.76 f 0.02 A.,ICF = 1.40 f 0.03A.; LCI-C-F = 110 f 2'. TABLEI11 INERTIA (IN AT. WT. X



CH2C12.16 The lowering of the coupling constant may result partly from increased double-bond character and partly from increased ionic character" of the C-C1 bond. Discussion

The structure is essentially in agreement with the electron diffraction results and is compatible with Atomic weights used: C, 12.00382; H, 1.008123; Cls5, those of the other halogenated methanes. The 34.97867; C P . 36.97750;. F, most striking feature is the marked shortening of . 19.00450 CHtCI"F CHrClI'F the C-CI: bond as compared to molecules not conI , 12.0891 12.1099 taining fluorine; the observed value is in line with Ib 88.4311 90.573, that of 1.74 A. calculated for C F C l by Sheridan I e 97.3029 99.4660 and The quadrupole data indicate that the shortening of both carbon-halogen bonds is Quadrupole Coupling.-If it is assumed that the probably due largely to contributions of the resoC-Cl bond coincides with the z-principal axis of nance forms the quadrupole coupling dyadic, a transformation of axes may be used to find the components of the dyadic in its principal system. The other two axes H-k=Cl+ and H-C C1must lie in the plane of symmetry (x-axis), and perpendicular to it (y-axis). The result, using the ClS6data, is xxx = 31.63 Mc., xyy = 38.83 Mc., xz, = -70.46 Mc., all f1 Mc. Independent data postulated by P a ~ l i n g . ' ~Inductive effects in the were not obtained for the other isotope, the ratio of carbon-halogen Fonds may also contribute to the 1:1.268812for the coupling constants in CI3' to variation in length (see ref. 4, footnote 15). The those in C136being used in predicting the fine struc- relative importance of these and possibly other ture. effects will evidently be debatable until a rigorous Following Dean13 an estimate of the fractional quantum-mechanical approach becomes possible. double-bond character, f,of the C-Cl bond may be Acknowledgments.-It is a pleasure to acmade from the relation 3f/(2 - f) = (xxx - xyy)/ the unfailing help and encouragement of xzr. The result is 6.6%) in agreement with the ob- knowledge served bond shortening, and with Pauling's esti- Professor E. Bright Wilson, Jr., who suggested this research. Thanks are also due to Dr. E. K. mate14from the diffraction data.. The value of x.. may be compared with that of Plyler for a preliminary value of the parameter c) obtained from the infrared spectrum -75.13 reported for CH8C1l5 and of -78.4 for a - l/z(b of CH2ClF, which was helpful in the analysis. (12) R.L. Livingston, P h y s . Rev., 82, 289 (1951). (13) C. Dean, Thesis, Harvard University, 1952. Especially Chap. CAMBRIDGE, MASS. MOMENTSOF







See also J. H. Goldstein and J. K. Bragg, P h y s . Rev., 78, 346 (1950). (14) L.Pauling, "The Nature of the Chemical Bond," second edition, Cornell University Press, Ithaca, N. Y., 1945,p. 235. (15) W. Gordy. J. W. Simmons and A. G. Smith, Phys. Rev., 74, 243 (1948). 111.

(16) R. J. Myers and W. D. Gwinn, J. Chcm. Phys., 20, 1420 (1952). (17) C. H. Townes and B . P. Dailey, i b i d . , 17, 782 (1949). (18) J. Sheridan and W. Gordy, ibid., 20, 591 (1952). The calculations are based on assumed F-C-F angles of 108'.